A 2.00g sample of SX6(g) has a volume of 329.5mL at 1.00 atm and 20celsius. Identify element X. Name the compound.

Get the number of moles from the ideal gas law.

Then, knowing it was 2grams, you can get the mole mass. Subtract from that the mass of an S atom, the remainder is six X masses.

thank you I finally got it

the ans, is 45.6

To identify the element X and name the compound, we need to use the given information about the sample's properties and perform some calculations.

First, let's convert the given volume from milliliters (mL) to liters (L) and the temperature from Celsius to Kelvin (K).

329.5 mL * (1 L / 1000 mL) = 0.3295 L
20 Celsius + 273.15 = 293.15 K

To find the number of moles (n) of the sample, we can use the ideal gas law equation:

PV = nRT

Where:
P = Pressure (1.00 atm)
V = Volume (0.3295 L)
n = number of moles (unknown)
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (293.15 K)

Rearranging the equation to solve for n:

n = PV / RT

n = (1.00 atm) * (0.3295 L) / (0.0821 L·atm/(mol·K) * 293.15 K)

After performing the calculation, we obtain the number of moles (n) in the sample.

Next, we need to determine the molar mass of the compound SX6 to identify the element X.

Molar mass is calculated by dividing the mass of the sample by the number of moles:

Molar mass = mass / moles

Given the mass of the sample is 2.00 g, and the number of moles (n) is calculated in the previous step, we can find the molar mass.

Finally, using the molar mass and periodic table, we can identify the element X based on its atomic mass.

Additionally, knowing the elements involved, we can name the compound SX6 by using the naming conventions for molecular compounds.

By following these steps and performing the calculations, we can identify the element X and name the compound correctly.